Fining agents for silicate glasses

ABSTRACT

A fining agent for reducing the concentration of seeds or bubbles in a silicate glass. The fining agent includes at least one inorganic compound, such as a hydrate or a hydroxide that acts as a source of water. In one embodiment, the fining agent further includes at least one multivalent metal oxide and, optionally, an oxidizer. A fusion formable and ion exchangeable silicate glass having a seed concentration of less than about 1 seed/cm 3  is also provided. Methods of reducing the seed concentration of a silicate glass, and a method of making a silicate glass having a seed concentration of less than about 1 seed/cm 3  are also described.

CROSS-REFERENCE TO RELATED APPLICATIONS

This application is a continuation of U.S. application Ser. No. 14/146,377 filed Jan. 2, 2014, which is a divisional of U.S. application Ser. No. 13/346,235, filed Jan. 9, 2012, which is a divisional of U.S. application Ser. No. 12/392,577 (now U.S. Pat. No. 8,158,543), and claims the benefit of U.S. Provisional Application Ser. No. 61/067,130 filed on Feb. 26, 2008, the contents of which are incorporated by reference herein in their entirety.

BACKGROUND

During glass formation from the melt, contaminants in the melt tend to form gas bubbles, also referred to in the art as “seeds.” Such seeds affect the performance and quality of the glass, and efforts are made to remove or “fine” them from the glass.

Seed formation is problematic for silicate glasses. In particular, aluminosilicate glasses and other silicate glasses that melt at high temperature are much more difficult to fine than other glasses. The high viscosities of such glasses slow the rate of bubble removal by via Stokes fining; i.e., allowing the bubbles to rise to the surface of the melt due to buoyancy.

Fining agents such as As₂O₃, Sb₂O₃, and halides have been used to remove bubbles from aluminosilicate glasses. These chemical fining packages work by releasing gas to existing bubbles, causing them to increase in size and rise more quickly to the top of the melt. However, these components are toxic, hazardous to handle, expensive, and undesirable for environmentally green products and processes. Sulfate fining agents have also been used in soft glasses. However, they contribute to sulfur emissions and actually exacerbate seed formation in aluminosilicate glasses.

SUMMARY

Environmentally friendly fining agents for reducing the concentration of seeds or bubbles in a silicate glass are provided. The fining agent includes at least one inorganic compound, such as a hydrate or a hydroxide, which acts as a source of water. In one embodiment, the fining agent further includes at least one multivalent metal oxide and, optionally, an oxidizer. A fusion formable and ion exchangeable silicate glass having a seed concentration of less than about 1 seed/cm3 is also provided. Methods of reducing the seed concentration of a silicate glass, and a method of making a silicate glass having a seed concentration of less than about 1 seed/cm3 are also described.

Accordingly, one aspect of the disclosure is to provide a silicate glass. The silicate glass has a seed concentration of less than about 1 seed/cm³, wherein a batch or raw materials that form the silicate glass includes at least one fining agent. The fining agent comprises at least one inorganic compound that acts as of a source of water at a temperature where a melt is formed.

Another aspect of the disclosure is to provide a fining agent for silicate glasses. The fining agent comprises an inorganic compound that acts as of a source of water at a temperature where a melt is formed, wherein the water vaporizes and expands existing bubbles in the melt and allows the expanded bubbles to rise to the surface of the melt and escape the melt to reduce the seed concentration in the silicate glass to less than about 1 seed/cm³.

A third aspect of the disclosure is to provide a method of reducing a concentration of seeds in a silicate glass. The method comprises the steps of: providing a batch comprising raw materials for the silicate glass and at least one fining agent, wherein the at least one fining agent comprises at least one inorganic compound that acts as of a source of water at a temperature where a melt is formed; melting the batch to form the melt; vaporizing the water to form water vapor, wherein the water vapor expands existing bubbles in the melt; allowing the expanded bubbles to rise to the surface of the melt and escape the melt to reduce the seed concentration in the melt below a predetermined concentration; and removing at least a portion of the coalesced bubbles and seeds from the melt.

A fourth aspect of the disclosure is to provide a method of making asilicate glass having a seed concentration of less than about 1 seed/cm³. The method comprises the steps of providing a batch comprising raw materials for the silicate glass and at least one fining agent, wherein the at least one fining agent comprises at least one inorganic compound that acts as of a source of water at a temperature of a melt; melting the batch to form the melt; vaporizing the water to form water vapor, wherein the water vapor expands existing bubbles in the melt; allowing the expanded bubbles to rise to the surface of the melt and escape the melt to reduce the seed concentration in the melt below a predetermined concentration; removing at least a portion of the coalesced bubbles and seeds from the melt; and solidifying the melt to form the silicate glass, wherein the silicate glass has a seed concentration of less than about 1 seed/cm³.

These and other aspects, advantages, and salient features will become apparent from the following detailed description, the accompanying drawings, and the appended claims.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1 is a photograph of polished cross sections of glasses obtained from melts containing fining agents;

FIG. 2 is a photograph of polished cross sections of glasses obtained from melts showing the effect of different fining agents on the concentration of seeds within the melt; and

FIG. 3 is a photograph of polished cross sections of glasses obtained from melts comparing the effectiveness of hydroxide fining agents in reducing seed formation.

DETAILED DESCRIPTION

In the following description, like reference characters designate like or corresponding parts throughout the several views shown in the figures. It is also understood that, unless otherwise specified, terms such as “top,” “bottom,” “outward,” “inward,” and the like are words of convenience and are not to be construed as limiting terms. In addition, whenever a group is described as comprising at least one of a group of elements and combinations thereof, it is understood that the group may comprise, consist of, or consist essentially of any number of those elements recited, either individually or in combination with each other. Similarly, whenever a group is described as consisting of at least one of a group of elements or combinations thereof, it is understood that the group may consist of any number of those elements recited, either individually or in combination with each other. Unless otherwise specified, a range of values, when recited, includes both the upper and lower limits of the recited range.

Referring to the drawings in general and to FIG. 1 in particular, it will be understood that the illustrations are for the purpose of describing particular embodiments and are not intended to limit the disclosure and appended claims thereto.

Glasses having relatively high viscosities (i.e., 200 Poise viscosities of between about 1500° C. and 1675° C.) may require melting to obtain a glass having low levels of inclusions. Gaseous inclusions, blisters, or bubbles, which are also referred to herein as “seeds,” tend to have an adverse affect of the optical quality and properties of the glass. For example, the presence of seeds affects the refractive index, density, and transmission of light through the glass. To aid in eliminating or reducing the concentration of these gaseous inclusions, it is, in some instances, useful to add chemical fining agents. Such fining agents fill early-stage bubbles with gas, thus increasing the velocity at which the bubbles rise through the melt. Typical fining agents include, but are not limited to: oxides of arsenic, antimony, tin and cerium; metal halides (fluorides, chlorides and bromides); metal sulfates; and the like. Arsenic oxides are particularly effective fining agents because they release oxygen very late in the melt stage. However, arsenic and antimony are generally regarded as hazardous materials. Therefore, it may be advantageous in particular applications to completely avoid using arsenic or antimony, and instead use a nontoxic component to produce a fining effect.

As described herein, the number of seeds within silicate glasses is reduced by providing fining agents that comprise at least one inorganic compound that acts as a source of water at a temperature of a melt formed by the mixture of raw materials (also referred to herein as the “batch” or “batch materials”) that are used to form the silicate glass. The inorganic compound may melt or decompose at a temperature below the temperature of the melt, generating water. The water is initially dissolved as a vapor in the melt. As the temperature of the melt increases, the water vapor comes out of solution and is captured by bubbles already present in the melt. The captured water vapor fills the bubbles with steam and expands the bubbles, causing them to rise more quickly to the surface of the melt and escape. For example, aluminum hydroxide (Al(OH)₃), which is used as a fining agent, decomposes to form boehmite (AlO.(OH)) and water at temperatures below those at which a melt initially appears. The boehmite will decompose at higher temperatures to form alumina (Al₂O₃) and water. The water produced by this two-step decomposition will eventually be captured by bubbles already present in the melt, increasing the size of these bubbles and causing them to rise to the surface of the melt, where they escape. The fining agent is also substantially free of arsenic and antimony.

In one embodiment, the water source comprises at least one of a hydrate, a metal hydroxide, and combinations thereof. Hydrates are solid inorganic compounds that contain water molecules, which are either bound to a metal or silicon center or crystallized with a metal complex. Such hydrates are said to contain “water of crystallization” or “water of hydration.” With the exception of boric acid, such hydrates may include hydrates of oxides or salts formed by any of the constituents (e.g., alumina, alkali and alkali earth metals, zirconium) of the silicate glass. Metal hydroxides are compounds that comprise a metal and the diatomic hydroxyl OH⁻ anion.

Non-limiting examples of inorganic or metal hydrates and hydroxides include, but are not limited to: phyllosilicates, such as clays and micas; zeolites; other hydrated silicates; and the like. Clays that may be used as a water source in the fining agent include, but are not limited to: aluminum silicate hydroxides, such as kaolinite and pyrophillite; talc (magnesium silicate hydroxide); montmorillonite-smectite (e.g., Bentonite); and combinations thereof, such as clinochlore ((Mg₅Al)(AlSi₃)O₁₀(OH)₈). Zeolites are hydrated aluminosilicates having symmetrically stacked alumina and silica tetrahedra that form an open, stable, three-dimensional honeycomb structure having a negative charge. Zeolites that may be used as a water source in the fining agent include, but are not limited to: mineral zeolites, such as analcime, chabazite, heulandite, natrolite, phillipsite, stilbite, and mordenite. Natrolite (Na₂Al₂Si₃O₁₀.2H₂O) has a formula that is typical of such mineral zeolites. Synthetic zeolites such as zeolite A, ZSM-5, and the like may also be used in the fining agent.

In one embodiment, the fining agent includes at least one metal hydroxide. Such hydroxides may include the hydroxides formed by any of the constituents (e.g., alumina ((Al(OH)₃); alkali (e.g., NaOH, KOH, LiOH) and alkali earth (Mg(OH)₂, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂) metals; and zirconium (Zr(OH)₄)) of the silicate glass. Additionally, the fining agent may comprise the mineral hydroromarchite (Sn₃O₂(OH)₂), and/or hydroxides of zinc (Zn(OH)₂) and gallium (Ga(OH)₃).

In another embodiment, the fining agent further includes at least one multivalent metal oxide that acts as a source of oxygen to the melt and, optionally, an oxidizer. These multivalent metal oxides are reduced in the glass melt, releasing oxygen, which may also form bubbles. Non-limiting examples of such oxides include, but are not limited to, tin(IV) oxide (SnO₂), ceria or cerium oxide (CeO₂), and the like. The fining agent, in one embodiment, comprises up to 0.5 mol % SnO₂, up to 0.5 mol % CeO₂, and, optionally, 0-4 mol % of oxidizer.

Oxidizers such as, but not limited to, aluminum nitrate, alkali metal nitrates, alkali earth metal nitrates, zirconium nitrate, ammonium nitrate, and the like re-oxidize the multivalent metal oxides in the melt, thus enhancing the effectiveness of the fining agent. Rather than be consumed by tramp contaminants and organic compounds, the oxygen produced by the reduction of multivalent metal oxides such as tin(IV) oxide and ceria are absorbed by the oxidizer and reused in the fining process.

The fining agents described herein are “batched in” with the rest of the raw materials that are used to formulate the silicate glass. The inorganic compounds that are added as sources of water, such as the hydrates and hydroxides, upon release of water, form oxides that account for a portion of the glass composition.

The source of water decomposes to release water, which is first dissolved in the initial melt and later comes out of solution and vaporizes into the melt as steam (water vapor). The steam is captured by bubbles that are generated by impurities and already exist in the melt. The steam fills these existing bubbles, causing them to expand and increase in size. The larger bubbles rise more quickly to the top surface of the melt and escape the melt. Each mole of aluminum hydroxide, for example, decomposes in the melt to first form boehmite, which then decomposes to form alumina (aluminum oxide), ultimately releasing 1.5 moles of water according to the reactions Al(OH)₃→AlO.(OH)+H₂O, and AlO.(OH)→½Al₂O₃+½H₂O. Expressed in terms of the amount of alumina that is initially introduced, or batched, into the glass as aluminum hydroxide, each mole of Al₂O₃ that is batched provides 3 moles of water vapor to the melt. Given that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure (1 kPa (1 bar) pressure, 273 K), or STP, each mole of Al₂O₃ batched as Al(OH)₃ (molecular weight 156 grams) releases 67 liters of gas. Because the gas is released at the temperature of the melt, the actual volume of gas released by each mole of alumina batched as Al(OH)₃ will be much greater than 67 liters. At 1000° C. (1273 K), for example, each mole of alumina batched as Al(OH)₃ releases a volume of about 312 liters of gaseous water.

Similarly, a mole of sodium hydroxide decomposes to form sodium oxide and water vapor according to the reaction NaOH→½Na₂O+½H₂O. The amount Na₂O batched as sodium hydroxide provides one mole of water vapor to the melt. At STP, one mole of a gas has a volume of 22.4 liters. As previously described above, gaseous water is released at the temperature of the melt, and the actual volume of gas released by each mole of sodium oxide batched as NaOH will be much greater than 22.3 liters.

In one embodiment, at least 1 mole of water per kilogram of glass is used to effectively “fine” the glass—i.e., reduce the number of seeds or bubbles in the glass. In another embodiment, 5-50 moles H₂O/kg of glass are used to fine the glass. The amount of water needed to fine the glass depends in part on the density of the glass and other factors, such as the composition of the glass and the viscosity and temperature of the melt. Depending on the parameters for a particular glass, it may be possible in some instances to use less than 1 mole H₂O/kg glass to effectively fine the glass.

The fining agents described herein are capable of providing at least 0.25 moles, and, in one embodiment, 0.5 moles of gas (water vapor, oxygen, or the like), per mole of fining agent to the melt. The fining agents are capable of producing a seed concentration within the silicate glass of less than about 1 seed/cm³ or, alternatively, about 5 seeds per pound (454 grams) of silicate glass. In one embodiment, the fining agents described herein are capable of producing a silicate glass that is substantially free of seeds.

The fining agents described herein may also act as “fugitive” fluxes that reduce the viscosity of the melt, causing the bubbles to rise to the top of the melt more rapidly.

A silicate glass having a seed concentration of less than about 1 seed/cm³ or, alternatively, about 5 seeds per pound (454 grams) of silicate glass, is also provided. In one embodiment, the silicate glass is substantially free of seeds. At least one of the fining agents described hereinabove is added to a batch comprising raw materials for the silicate glass. Such raw materials for making the silicate glasses described herein are known in the art. After adding the at least one fining agent to the batch, the batch is melted. The fining agent comprises at least one inorganic compound that acts as a source of water at a temperature of a melt. The silicate glass may be one of a soda lime glass, a borosilicate glass, an aluminosilicate glass, and combinations thereof, such as, for example an aluminoborosilicate glass.

In one embodiment, the silicate glass comprises: 60-70 mol % SiO₂; 6-14 mol % Al₂O₃; 0-15 mol % B₂O₃; 0-15 mol % Li₂O; 0-20 mol % Na₂O; 0-10 mol % K₂O; 0-8 mol % MgO; 0-10 mol % CaO; 0-5 mol % ZrO₂; 0-1 mol % SnO₂; 0-1 mol % CeO₂, wherein 12 mol % ≤Li₂O+Na₂O+K₂O ≤20 mol % and 0 mol %≤MgO+CaO≤10 mol %. In another embodiment, the silicate glass comprises: 63.5-66.5 mol % SiO₂; 8-12 mol % Al₂O₃; 0-3 mol % B₂O₃; 0-5 mol % Li₂O; 8-18 mol % Na₂O; 0-5 mol % K₂O; 1-7 mol % MgO; 0-2.5 mol % CaO; 0-3 mol % ZrO₂; 0.05-0.25 mol % SnO₂; 0.05-0.5 mol % CeO₂, wherein 14 mol %≤Li₂O+Na₂O+K₂O≤18 mol % and 2 mol %≤MgO+CaO≤7 mol %.

The largest single constituent of the silicate glass is SiO₂, which forms the matrix of the glass and is present in the inventive glasses in a concentration ranging from about 60 mol % up to and including about 70 mol %. SiO₂ serves as a viscosity enhancer that aids formability and imparts chemical durability to the glass. At concentrations that are higher than the range given above, SiO₂ prohibitively raises the melting temperature. Glass durability suffers at concentrations below the 60-70 mol % SiO₂ range. In addition, lower SiO₂ concentrations can cause the liquidus temperature to increase substantially in glasses having high alkali or alkali earth oxide concentrations.

The greater alkali metal oxide content of the silicate glass facilitates melting, softens the glass, enables ion exchange, decreases melt resistivity, and breaks up the glass network, which increases thermal expansion and decreases durability. Mixtures of alkali metal oxides help depress the liquidus temperature and may enhance ion exchange as well. While Li₂O provides fast ion exchange, low density, and high modulus, it is also quite expensive. Na₂O is very desirable for ion exchange with K⁺ ions for chemical strengthening and makes stable glasses with respect to devitrification. Small amounts of K₂O relative to Na₂O actually help increase the rate exchange of K⁺ ions for Na⁺ ions and decrease the liquidus temperature, but also increase the thermal expansivity of the glass.

Alumina (Al₂O₃) and, to a lesser extent, zirconia (ZrO₂) have the opposite effect of the alkali metal oxides. In addition, Al₂O₃ scavenges non-bridging oxygens (NBOs) to form AlO₄ tetrahedra while making the glass thermally harder. Alumina and zirconia also provide lower expansion and greater durability but, at high concentrations, make the glass more difficult to melt. In most ion exchangeable glasses, R₂O>Al₂O₃ (where R₂O represents at least one alkali metal oxide, such as Li₂O, Na₂O, K₂O) since glasses in which R₂O=Al₂O₃ are very difficult to melt unless B₂O₃ is present.

Alkaline earth oxides help create a steeper viscosity curve for the glasses. Replacing alkali metal oxides with alkaline earth metal oxides generally raises the anneal and strain points of the glass while lowering the melting temperatures needed to make high quality glass. MgO and CaO are less expensive than SrO and BaO and do not increase the density as much as the heavier oxides. BaO is also considered to be a hazardous or toxic material, and its presence is therefore undesirable. Accordingly, in one embodiment, the glass is substantially free of barium. Large amounts of MgO tend to increase the liquidus temperature, as the oxide is prone to form forsterite (Mg₂SiO₄) at low MgO concentrations in sodium aluminosilicate glasses. Accordingly, in some embodiments, the silicate glass described herein comprises 0-8 mol % MgO.

B₂O₃ may be used as a flux to soften glasses, making them easier to melt. B₂O₃ also helps scavenge non-bridging oxygen atoms (NBOs), converting the NBOs to bridging oxygen atoms through the formation of BO₄ tetrahedra, which increases the toughness of the glass by minimizing the number of weak NBOs. B₂O₃ also lowers the hardness of the glass which, when coupled with the higher toughness, decreases the brittleness, thereby resulting in a mechanically durable glass.

Arsenic and antimony are widely regarded as hazardous or toxic materials, and their presence is therefore undesirable. Accordingly, the silicate glass, in another embodiment, is substantially free of at least one of arsenic, antimony, and barium.

In one embodiment, the silicate glass has a liquidus viscosity of at least 100 kilopoise (kpoise). In another embodiment, the liquidus viscosity is at least 160 kpoise, and, in a third embodiment, the liquidus viscosity is at least 220 kpoise. As used herein, the term “liquidus viscosity” refers to the viscosity of a molten glass at the liquidus temperature, wherein the liquidus temperature refers to the temperature at which the very last crystals melt away as temperature is increased from room temperature. These properties permit these silicate glasses to be down-drawable; i.e., the glass is capable of being formed into sheets using down-draw methods such as, but not limited to, fusion draw and slot draw methods that are known to those skilled in the art. Such down-draw processes are used in the large-scale manufacture of ion-exchangeable flat glass.

The fusion draw process uses a drawing tank that has a channel for accepting molten glass raw material. The channel has weirs that are open at the top along the length of the channel on both sides of the channel. When the channel fills with molten material, the molten glass overflows the weirs. Due to gravity, the molten glass flows down the outside surfaces of the drawing tank. These outside surfaces extend down and inwardly so that they join at an edge below the drawing tank. The two flowing glass surfaces join at this edge to fuse and form a single flowing sheet. The fusion draw method offers the advantage that, since the two glass films flowing over the channel fuse together, neither outside surface of the resulting glass sheet comes in contact with any part of the apparatus. Thus, the surface properties of the glass sheet are not affected by such contact.

The slot draw method is distinct from the fusion draw method. Here the molten raw material glass is provided to a drawing tank. The bottom of the drawing tank has an open slot with a nozzle that extends the length of the slot. The molten glass flows through the slot/nozzle and is drawn downward as a continuous sheet therethrough and into an annealing region. Compared to the fusion draw process, the slot draw process provides a thinner sheet, as only a single sheet is drawn through the slot, rather than two sheets being fused together, as in the fusion down-draw process.

Down-draw processes produce surfaces that are relatively pristine. Because the strength of the glass surface is controlled by the amount and size of surface flaws, a pristine surface that has had minimal contact has a higher initial strength. When this high strength glass is then chemically strengthened, the resultant strength is higher than that of a surface that has been lapped and polished. Chemical strengthening or tempering by ion exchange also increases the resistance of the glass to flaw formation due to handling. Down-drawn glass may be drawn to a thickness of less than about 2 mm. In addition, down drawn glass has a very flat, smooth surface that can be used in its final application without costly grinding and polishing.

In one embodiment, the silicate glass described herein is substantially free of lithium. As used herein, “substantially free of lithium” means that lithium is not intentionally added to the glass or glass raw materials during any of the processing steps leading to the formation of the alkali aluminosilicate glass. It is understood that a silicate glass or a silicate glass article that is substantially free of lithium may inadvertently contain small amounts of lithium due to contamination. The absence of lithium reduces poisoning of ion exchange baths, and thus reduces the need to replenish the salt supply needed to chemically strengthen the glass. In addition, due to the absence of lithium, the glass is compatible with continuous unit (CU) melting technologies such as the down-draw processes described above and the materials used therein, the latter including both fused zirconia and alumina refractories and zirconia and alumina isopipes.

In one embodiment, the silicate glass comprises at least one alkali metal oxide and is ion exchangeable. As used herein, the term “ion-exchangeable” is understood to mean that the glass is capable of being strengthened by ion exchange processes that are known to those skilled in the art. Such ion exchange processes include, but are not limited to, treating the heated alkali aluminosilicate glass with a heated solution containing ions having a larger ionic radius than ions that are present in the glass surface, thus replacing the smaller ions with the larger ions. Potassium ions, for example, could replace sodium ions in the glass. Alternatively, other alkali metal ions having larger atomic radii, such as rubidium or cesium, could replace smaller alkali metal ions in the glass. Alternatively, the smaller alkali metal ions could be replaced by Ag⁺ ions. Similarly, other alkali metal salts such as, but not limited to, sulfates, halides, and the like may be used in the ion exchange process. In one embodiment, the down-drawn glass is chemically strengthened by placing it in a molten salt bath comprising KNO₃ for a predetermined time period to achieve ion exchange. In one embodiment, the temperature of the molten salt bath is about 430° C. and the predetermined time period is about eight hours.

Surface compressive stress refers to a stress caused by the substitution during chemical strengthening of an alkali metal ion contained in a glass surface layer by another alkali metal ion having a larger ionic radius. In one embodiment, potassium ions are substituted for sodium ions in the surface layer of the glass described herein. The glass has a surface compressive stress of at least about 200 MPa. In one embodiment, the surface compressive stress is at least about 600 MPa. The alkali aluminosilicate glass has a compressive stress layer that has a depth of at least about 30 μm and, in another embodiment, the depth of the compressive stress layer is at least about 40 μm.

The replacement of smaller ions by larger ions at a temperature below that at which the glass network can relax produces a distribution of ions across the surface of the glass that results in a stress profile. The larger volume of the incoming ion produces compressive stress (CS) on the surface and tension in the center (central tension, or CT) of the glass. The compressive stress is related to the central tension by the following relationship: CS=CT×(t−2DOL)/DOL; where t is the thickness of the glass and DOL is the depth of exchange, also referred to as depth of layer.

The silicate glasses described herein are resistant to both chipping and scratching, making it well suited for use in cover plates, touch screens, watch crystals, solar concentrators, windows, screens, containers, and other applications that require strong and tough glass with good scratch resistance.

A method of reducing the concentration of seeds in a silicate glass is also provided. A batch comprising raw materials for the silicate glass and at least one fining agent, as described herein, is first provided. Such raw materials include, but are not limited to, sand, alumina, nepheline syenite (a mineral comprising Na₂O.Al₂O₃.2SiO₂), boric acid, soda ash, potassium carbonate, magnesia, limestone, and the like. The batch containing the at least one fining agent is then melted to form a silicate glass melt. The fining agent comprises at least one inorganic compound that acts as a source of water at the temperature of the melt. In one embodiment, the fining agent comprises at least one of a metal hydrate, a metal hydroxide, and combinations thereof. In another embodiment, the fining agent may further include at least one multivalent metal oxide that acts as a source of oxygen to the melt and, optionally, at least one oxidizer, all of which have been previously described herein.

As previously described herein, the inorganic compound that acts as source of water at the temperature of the melt may decompose below the temperature of the melt, generating water vapor that is initially dissolved in the solid or melt. As temperature increases the water vapor (steam) comes out of solution. The water vapor is captured by bubbles that already exist in the melt. The water vapor fills these existing bubbles, causing them to expand and increase in size. The expanded bubbles rise more quickly to the top surface of the melt and escape the melt. At least a portion of the expanded bubbles are then removed from the melt, usually by allowing them to rise to the surface of the melt, where the gases in the bubbles escape into the atmosphere above the melt and the seed concentration in the resulting silicate glass is reduced to a concentration below a predetermined level. In one embodiment, the bubbles are allowed to rise and the gases allowed to escape by maintaining the temperature of the melt at or above a predetermined temperature. For example, some aluminosilicate glasses are first melted at about 1525° C. and then heated to about 1600° C. to allow gases to escape from the melt.

A method of making the silicate glasses described herein is also provided. A batch comprising raw materials for a silicate glass and at least one fining agent, as described herein, is first provided. Such raw materials include, but are not limited to, sand, alumina, nepheline syenite (a mineral comprising Na₂O.Al₂O₃.2SiO₂), boric acid, soda ash, potassium carbonate, magnesia, limestone, and the like. The batch containing the at least one fining agent is then heated to a temperature at which a melt begins to form. The fining agent comprises at least one inorganic compound that acts as of a source of water at the temperature of the melt. In one embodiment, the fining agent comprises at least one of a metal hydrate and a metal hydroxide. In another embodiment, the fining agent may further include at least one multivalent metal oxide that acts as a source of oxygen to the melt and, optionally, at least one oxidizer, all of which have been previously described herein.

As previously described herein, the inorganic compound that acts as source of water at the temperature of the melt may decompose below the temperature of the melt, generating water vapor that is initially dissolved in the solid or melt. As temperature increases, the water vapor (steam) comes out of solution. The water vapor is captured by bubbles that already exist in the melt. The water vapor fills these existing bubbles, causing them to expand and increase in size. The expanded bubbles rise more quickly to the top surface of the melt and escape the melt. At least a portion of the expanded bubbles are then removed from the melt, usually by allowing them to rise to the surface of the melt where the gases in the bubbles escape into the atmosphere above the melt, thus reducing the concentration of bubbles or seeds in the melt to a concentration below a predetermined level. In one embodiment, the bubbles are allowed to rise and the vapors allowed to escape by maintaining the temperature of the melt above a predetermined temperature. The silicate glass, having a seed concentration of less than about 1 seed/cm³, is then solidified.

EXAMPLES

The following examples illustrate the features and advantages of the invention and in no way are intended to limit the disclosure and appended claims thereto.

Example 1

Example 1 serves to illustrate the effectiveness of the fining agents described herein. Nine samples of aluminosilicate crucible melts were prepared. The batch materials used for each sample are listed in Table 1a. Different combinations of the fining agents of the present invention were added to samples 11-18. Sample 19 did not contain any of the fining agents described hereinabove, and thus served as a control sample. In samples 12, 13, 14, and 18, the fining agent aluminum hydroxide (Al(OH)₃) was substituted for alumina (Al₂O₃) in the batch. Sodium hydroxide (NaOH) was substituted for soda ash in samples 15 and 16. Ceria and tin(IV) oxide were added to samples 11-18, and the oxidizer sodium nitrate (NaNO₃) was added to samples 17 and 18.

The batched samples were melted at 1525° C. for one hour and then heated at 1600° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 1b and 1c, respectively. Tables 1b and 1c also include the averages concentration of seeds or bubbles in the glass samples, expressed as seeds/cm³.

As previously described herein, upon the release of water, the inorganic compound fining agents, such as the hydrates and hydroxides that are added as sources of water, form oxides that account for a portion of the glass composition. This is shown in tables 1c, 2c, and 3c.

Polished cross-sections of glasses obtained from the melts in Example 1 are shown in FIG. 1. Sample 19, which contained none of the fining agents, has an average seed concentration of 930 seeds/cm³. The addition of 0.1 mol % SnO₂ and 0.1 mol % CeO₂ alone (sample 11) drastically reduces the concentration of seeds or bubbles in the glass to 79.1 seeds/cm³. The use of the oxidizer (NaNO₃) with SnO₂ and CeO₂ alone (sample 17) also further reduces the concentration of bubbles or seeds to 0.061 seeds/cm³.

The addition of either Al(OH)₃ (samples 12, 13, 14, 18), or NaOH (samples 15 and 16) adds water in the form of hydroxides. Either of these fining agents reduces the seed concentration to levels below those observed when a combination of tin(IV) oxide and ceria alone (sample 11) is used, whereas addition of even higher levels of these hydroxides virtually eliminate seeds or bubbles under the melting conditions used. The addition of Al(OH)₃ reduces the seed concentration to values ranging from 0.610 seeds/cm³ (sample 14, in which 359 g of nephelene syenite were added to the batch) to 0.183 seeds/cm³ (sample 18, in which 247 g (Al(OH)₃ were added to the batch). The addition of NaOH reduces seed concentration to values ranging from 0.580 seeds/cm³ (sample 15, 87 g NaOH added to the batch) to 0.677 seeds/cm³ (sample 16, 173 g NaOH added to the batch). Use of the oxidizer NaNO₃ with SnO₂, CeO₂, and a hydrate (sample 18) reduces the number of bubbles/seeds in the glass to a concentration of 0.183 seeds/cm³.

Example 2

Example 2 illustrates the amount of fining agent (or agents) that effectively reduce the concentration of bubbles/seeds in silicate glasses. Nine samples of aluminosilicate crucible melts were prepared. The batch materials used for each sample are listed in Table 2a. Ceria and tin(IV) oxide were added to samples 21-29, and are the only fining agents present in sample 29. The fining agent aluminum hydroxide (Al(OH)₃) was substituted for alumina (Al₂O₃) in the batch in samples 21 and 22, and sodium hydroxide (NaOH) was substituted for soda ash in samples 23 and 24. Samples 21 and 23 each contain an amount of hydroxide fining agent (Al(OH)₃ in sample 21 and NaOH in sample 23) to generate three moles of H₂O, whereas samples 22 and 24 each contain an amount of hydroxide fining agent ((Al(OH)₃) in sample 21 and NaOH in sample 23) to generate six moles of H₂O. Sodium nitrate was added as an oxidizer to samples 27 and 28.

Varying amounts of tall oil, an organic fatty acid, were added to samples 25 and 26. Tall oil burns at melt temperatures, consuming O₂ to yield CO, CO₂, and water as combustion products.

The batched samples were melted at 1525° C. for one hour and then heated at 1600° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 2b and 2c, respectively.

Polished cross-sections of glasses obtained from the melts in Example 2 are shown in FIG. 2. Both aluminum hydroxide and sodium hydroxide fining agents effectively fine the glass. For a given amount of water generated by the fining agents (i.e., comparing sample 21 vs. sample 23 and sample 22 vs. sample 24), NaOH appears to be more effective than Al(OH)₃ in reducing the bubble/seed count in the glass.

Based on these experiments, tall oil does not act as a fining agent. Instead, as seen in samples 25 and 26 in FIG. 2, the addition of tall oil to the melt leads to an increase bubble/seed formation in the glass.

Example 3

Example 3 compares the effectiveness of the hydroxide fining agents to hydrogen permeation. The batch materials used for each sample are listed in Table 3a.

Samples 31 and 32 were identical samples, each containing aluminum hydroxide, tin(IV) oxide, and ceria. Samples 31 and 32 were placed in platinum crucibles. Sample 32 was melted with glass on both sides of the crucible to effectively shut off hydrogen permeation into the sample. Sample 32 was further contained by a second refractory crucible backer.

Samples 33 and 34 were identical samples, containing tin(IV) oxide, ceria, and 52.78 g of sodium nitrate oxidizer. Sample 33 was melted with glass on both sides of the crucible to effectively shut off hydrogen permeation into the sample. Samples 35, 36, and 37 contained SnO₂, CeO₂, and 26.39, 105.55 g, and 52.78 g, respectively, of NaNO₃. Sample 38 contained SnO₂ and NaNO₃, but no ceria, whereas sample 9 contained ceria and NaNO₃, but no tin(IV) oxide.

The batched samples were melted at 1525° C. for one hour and then heated at 1600° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 3b and 3c, respectively.

Polished cross-sections of glasses obtained from the melts in Example 3 are shown in FIG. 3. Comparison of samples 31 and 32 shows no apparent difference in the number of bubbles/seeds, indicating the hydrogen permeation is not the mechanism for fining/bubble reduction in the melt.

Samples 33 and 34 do not contain hydride fining agents. In this case, the glass where H₂ permeation was shut off (sample 33) has fewer bubbles, again showing that H₂ permeation is not the effective mechanism of the fining package of the present invention.

Samples 35-37 demonstrate that varying the amount of oxidizer has little effect on the number of bubbles/seeds in the melt. These samples all exhibit low concentrations of bubbles/seeds, compared to glasses that do not contain the fining agents described herein (see, for example, sample 39 in FIG. 1). Similarly, melts containing oxidizer and either tin(IV) oxide alone (sample 38) or ceria alone (sample 39) yield low concentrations of bubbles/seeds, showing that the presence of just one of these fining agents and an oxidizer is still effective in removing bubbles/seeds.

Example 4

Example 4 identified fining agent or agents that effectively reduces the concentration of bubbles/seeds in soda lime glasses. Nine samples of soda lime crucible melts were prepared. The batch materials used for each sample are listed in Table 4a.

The batched samples were melted at 1425° C. for one hour and then heated at 1525° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 4b and 4c, respectively.

Sample 41, which contained no fining agent or oxidizer, had numerous seeds. A substantial reduction in seed concentration was observed in sample 48, in which talc and tin(IV) oxide were added to the batch. Lesser reductions in seed concentration was observed in samples 42 (containing only one fining agent: tin(IV) oxide); 43 (containing tin(IV) oxide and sodium nitrate oxidizer); 44 (containing only one fining agent: NaOH); 45 (containing tin(IV) oxide and NaOH); 46 (containing tin(IV) oxide, NaOH and sodium nitrate); 47 (containing tin(IV) oxide and calcium hydroxide); and 49 (containing tin(IV) oxide and sodium sulfate oxidizer).

Example 5

Example 5 identified fining agent or agents that effectively reduces the concentration of bubbles/seeds in aluminosilicate glasses that are used in liquid crystal display (LCD) applications. Nine samples of aluminosilicate crucible melts were prepared. The batch materials used for each sample are listed in Table 5a.

The batched samples were melted at 1550° C. for one hour and then heated at 1625° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 5b and 5c, respectively.

Very few seeds were observed in sample 54, in which fining agents aluminum hydroxide and tin(IV) oxide, and barium nitrate oxidizer were added to the batch. A substantial reduction in seed concentration was observed for samples 52 (containing tin(IV) oxide and half the amount of aluminum hydroxide in sample 54); 53 (containing tin(IV) oxide and the same amount of aluminum hydroxide as in sample 54); and 57 (containing sodium hydroxide, the same amount of aluminum hydroxide as in sample 54, and barium nitrate oxidizer). The reduction in seed concentration observed in samples 51 and 58 (both containing tin(IV) oxide and barium nitrate oxidizer) was less than that observed in samples 54, 52, 53, and 57, but still significant. No reduction in seed concentration was observed in samples 55 (containing twice the tin(IV) oxide concentration of samples 51-54 and 57-59, and barium nitrate) and 56 ((containing three times the tin(IV) oxide concentration of samples 51-54 and 57-59, and barium nitrate oxidizer).

Example 6

Example 6 identified fining agent or agents that effectively reduces the concentration of bubbles/seeds in aluminosilicate glasses having high boron concentrations. First and second sets of samples of crucible melts were prepared. The batch materials used for each of the first and second set of samples are listed in Table 5a1, respectively.

The first set of batched samples was melted at 1525° C. for one hour and then heated at 1625° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 5b1 and 5c1, respectively. The second set of batched samples was melted at 1529° C. for one hour and then heated at 1625° C. for one hour to facilitate the removal of bubbles from the melt. The compositions of the resulting glasses, expressed in weight percent and mole percent, are listed in Tables 5b2 and 5c2, respectively.

Samples 63 and 64 were substantially free of seeds. The batch material for sample 3 included fining agents tin(IV) oxide and hydrated alumina, whereas the batch material for sample 64 comprised fining agents arsenic pentoxide, tin(IV) oxide, and sodium nitrate as an oxidizer. The results obtained for samples 63 and 64 show that the addition of water (in the form of hydrated alumina) and tin(IV) oxide works as effectively as arsenic. A substantial reduction in seed concentration was also observed for samples 61 and 62, in which the batch materials included water (in the form of hydrated alumina) as the sole fining agent. The results obtained for samples 61 and 62 indicate that water-containing hydrates can effectively act as fining agents for glasses over a range of boron contents.

Substantial reduction in seed count were also observed for samples 65 and 66. Fining agents added to the batch materials for sample 65 included hydrated alumina, cerium oxide, and tin(IV) oxide. Fining agents added to the batch materials for sample 66 included hydrated alumina, sodium hydroxide, cerium oxide, and tin(IV) oxide. The results obtained for these samples also demonstrate the efficacy of water in the form of hydrated alumina as a fining agent for boron-containing glasses.

While typical embodiments have been set forth for the purpose of illustration, the foregoing description should not be deemed to be a limitation on the scope of the above disclosure and appended claims. Accordingly, various modifications, adaptations, and alternatives may occur to one skilled in the art without departing from the spirit and scope of the present disclosure.

TABLE 1a Compositions of batch materials, expressed in grams, for crucible melts described in Example 1. Batch Material 11 12 13 14 15 16 17 18 19 Sand 616.56 616.57 616.59 396.99 616.57 616.58 616.56 616.59 619.67 Alumina 161.71 82.33 0 0 161.71 161.71 161.71 0 162.51 Aluminum hydroxide 0.00 121.40 247.30 120.15 0.00 0.00 0.00 247.30 0.00 Nepheline Syenite 0.00 0.00 0.00 359.48 0.00 0.00 0.00 0.00 0.00 Boric Acid 12.06 12.06 12.06 12.06 12.06 12.06 12.06 12.06 12.06 Soda Ash 227.86 227.84 227.81 165.45 112.69 0 194.96 194.90 228.89 Sodium Hydroxide 0.00 0.00 0.00 0.00 87.27 172.67 0.00 0.00 0.00 Sodium Nitrate 0.00 0.00 0.00 0.00 0.00 0.00 52.78 52.78 0.00 Potassium Carbonate 52.69 52.69 52.69 27.29 52.69 52.69 52.66 52.66 52.98 Magnesia 37.86 37.86 37.86 37.92 37.87 37.87 37.86 37.86 38.07 Limestone 8.23 8.23 8.23 6.30 8.50 8.77 8.31 8.31 8.23 Tin (IV) Oxide 2.31 2.31 2.31 2.31 2.31 2.31 2.31 2.31 0.00 Cerium (IV) Oxide 2.72 2.72 2.72 2.72 2.72 2.72 2.72 2.72 0.00

TABLE 1b Compositions of glasses prepared from crucible melts described in Example 1, expressed in weight percent. Composition (mol %) 11 12 13 14 15 16 17 18 19 SiO₂ 61.37 61.37 61.38 61.38 61.37 61.37 61.37 61.37 61.69 Al₂O₃ 16.23 16.24 16.24 16.24 16.23 16.23 16.23 16.23 16.32 B₂O₃ 0.68 0.68 0.68 0.68 0.68 0.68 0.68 0.68 0.68 Na₂O 13.33 13.33 13.33 13.33 13.33 13.33 13.33 13.33 13.39 K₂O 3.57 3.57 3.57 3.57 3.57 3.57 3.57 3.57 3.59 MgO 3.66 3.66 3.66 3.66 3.66 3.66 3.66 3.66 3.68 CaO 0.50 0.50 0.50 0.50 0.50 0.50 0.50 0.50 0.50 SnO₂ 0.23 0.23 0.23 0.23 0.23 0.23 0.23 0.23 0.00 CeO₂ 0.27 0.27 0.27 0.27 0.27 0.27 0.27 0.27 0.00 Fe₂O₃ 0.02 0.02 0.01 0.01 0.02 0.02 0.02 0.01 0.02 Average seeds/cm³ 79.11 0.482 0.384 0.610 0.580 0.677 0.061 0.183 929.7

TABLE 1c Compositions of glasses prepared from crucible melts described in Example 1, expressed in mole percent. Composition (mol %) 11 12 13 14 15 16 17 18 19 SiO₂ 65.89 65.89 65.89 65.89 65.89 65.89 65.89 65.89 65.89 Al₂O₃ (Alumina) 10.27 5.27 0 0 10.27 10.27 10.27 0 10.27 Al₂O₃ (Al(OH)₃) 0 5 10.27 5 0 0 0 10.27 0 Al₂O₃ (Nepheline) 0 0 0 5.27 0 0 0 0 0 B₂O₃ 0.63 0.63 0.63 0.63 0.63 0.63 0.63 0.63 0.63 Na₂O (Soda Ash) 13.91 13.91 13.91 13.91 6.91 0 11.91 11.91 13.91 Na₂O (NaOH) 0 0 0 0 7 13.91 0 0 0 Na₂O (NaNO₃) 0 0 0 0 0 0 2 2 0 K₂O 2.45 2.45 2.45 2.45 2.45 2.45 2.45 2.45 2.45 MgO 5.86 5.86 5.86 5.86 5.86 5.86 5.86 5.86 5.86 CaO 0.57 0.57 0.57 0.57 0.57 0.57 0.57 0.57 0.57 SnO₂ 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0 CeO₂ 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0 Average seeds/cm³ 79.11 0.482 0.384 0.610 0.580 0.677 0.061 0.183 929.7

TABLE 2a Compositions of batch materials, expressed in grams, for crucible melts described in Example 2. Batch Material 21 22 23 24 25 26 27 28 29 Sand 616.56 616.56 616.56 616.56 616.56 616.56 616.56 189.49 616.56 Alumina 145.77 129.94 161.71 161.71 161.71 161.71 161.71 0 161.71 Aluminum hydroxide 24.22 48.59 0.00 0.00 0.00 0.00 0.00 0.00 0.00 Nepheline Syenite 0.00 0.00 0.00 0.00 0.00 0.00 0.00 699.16 0.00 Boric Acid 12.06 12.06 12.06 12.06 12.06 12.06 12.06 12.06 12.06 Soda Ash 227.86 227.85 178.50 129.15 227.86 227.86 194.96 73.63 227.86 Sodium Hydroxide 0.00 0.00 37.40 74.81 0.00 0.00 0.00 0.00 0.00 Sodium Nitrate 0.00 0.00 0.00 0.00 0.00 0.00 52.78 52.78 0.00 Potassium Carbonate 52.69 52.69 52.69 52.69 52.69 52.69 52.66 3.27 52.69 Magnesia 37.86 37.86 37.86 37.87 37.86 37.86 37.86 37.97 37.86 Limestone 8.23 8.23 8.35 8.46 8.23 8.23 8.31 4.56 8.23 Tin (IV) Oxide 2.31 2.31 2.31 2.31 2.31 2.31 2.31 2.31 2.31 Cerium (IV) Oxide 2.72 2.72 2.72 2.72 2.72 2.72 2.72 2.72 2.72 Fatty Acid, Tall Oil 1.00 5.00

TABLE 2b Compositions of glasses prepared from crucible melts described in Example 2, expressed in weight percent. Composition (wt %) 21 22 23 24 25 26 27 28 29 SiO₂ 61.38 61.37 61.37 61.37 61.37 61.37 61.37 61.38 61.37 Al₂O₃ 16.23 16.23 16.23 16.23 16.23 16.23 16.23 16.24 16.23 B₂O₃ 0.68 0.68 0.68 0.68 0.68 0.68 0.68 0.68 0.68 Na₂O 13.33 13.33 13.33 13.33 13.33 13.33 13.33 13.33 13.33 K₂O 3.58 3.57 3.57 3.57 3.57 3.57 3.57 3.57 3.57 MgO 3.66 3.66 3.66 3.66 3.66 3.66 3.66 3.66 3.66 CaO 0.50 0.50 0.50 0.50 0.50 0.50 0.50 0.50 0.50 SnO₂ 0.23 0.23 0.23 0.23 0.23 0.23 0.23 0.23 0.23 CeO₂ 0.27 0.27 0.27 0.27 0.27 0.27 0.27 0.27 0.27 Fe₂O₃ 0.02 0.02 0.02 0.02 0.02 0.02 0.02 0.00 0.02

TABLE 2c Compositions of glasses prepared from crucible melts described in Example 2, expressed in mole percent. Composition (mol %) 21 22 23 24 25 26 27 28 29 SiO₂ 65.89 65.89 65.89 65.89 65.89 65.89 65.89 65.89 65.89 Al₂O₃ (Alumina) 9.27 8.27 10.27 10.27 10.27 10.27 10.27 0 10.27 Al₂O₃ (Al(OH)₃) 1 2 0 0 0 0 0 0 0 Al₂O₃ (Nepheline) 0 0 0 0 0 0 0 10.27 0 B₂O₃ 0.63 0.63 0.63 0.63 0.63 0.63 0.63 0.63 0.63 Na₂O (Soda Ash) 13.91 13.91 10.91 7.91 13.91 13.91 11.91 11.91 13.91 Na₂O (NaOH) 0 0 3 6 0 0 0 0 0 Na₂O (NaNO₃) 0 0 0 0 0 0 2 2 0 K₂O 2.45 2.45 2.45 2.45 2.45 2.45 2.45 2.45 2.45 MgO 5.86 5.86 5.86 5.86 5.86 5.86 5.86 5.86 5.86 CaO 0.57 0.57 0.57 0.57 0.57 0.57 0.57 0.57 0.57 SnO₂ 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.10 CeO₂ 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.10

TABLE 3a Compositions of batch materials, expressed in grams, for crucible melts described in Example 3. Batch Material 31 32 33 34 35 36 37 38 39 Sand 616.59 616.59 616.56 616.56 616.56 616.56 188.45 616.76 616.36 Alumina 0 0 161.71 161.71 161.71 161.71 0 161.71 161.61 Aluminum hydroxide 247.30 247.30 0.00 0.00 0.00 0.00 0.00 0.00 0.00 Nepheline Syenite 0.00 0.00 0.00 0.00 0.00 0.00 699.16 0.00 0.00 Boric Acid 12.06 12.06 12.06 12.06 12.06 12.06 12.06 12.06 12.06 Soda Ash 227.81 227.81 194.96 194.96 211.41 162.05 73.33 194.97 194.78 Sodium Nitrate 0.00 0.00 52.78 52.78 26.39 105.55 52.78 52.78 52.78 Potassium Carbonate 52.69 52.69 52.66 52.66 52.67 52.64 3.15 52.66 52.66 Magnesia 37.86 37.86 37.86 37.86 37.86 37.86 37.97 37.86 37.86 Limestone 8.23 8.23 8.31 8.31 8.27 8.38 4.55 8.31 8.31 Tin (IV) Oxide 2.31 2.31 2.31 2.31 2.31 2.31 2.31 4.71 0.00 Cerium Oxide 2.72 2.72 2.72 2.72 2.72 2.72 2.72 0.00 5.35

TABLE 3b Compositions of glasses prepared from crucible melts described in Example 3, expressed in weight percent. Composition (wt %) 31 32 33 34 35 36 37 38 39 SiO₂ 61.38 61.38 61.37 61.37 61.37 61.37 61.38 61.40 61.36 Al₂O₃ 16.24 16.24 16.23 16.23 16.23 16.23 16.24 16.24 16.23 B₂O₃ 0.68 0.68 0.68 0.68 0.68 0.68 0.68 0.68 0.68 Na₂O 13.33 13.33 13.33 13.33 1333 13.33 13.33 13.33 13.32 K₂O 3.57 3.57 3.57 3.57 3.57 3.57 3.57 3.57 3.57 MgO 3.66 3.66 3.66 3.66 3.66 3.66 3.66 3.66 3.66 CaO 0.50 0.50 0.50 0.50 0.50 0.50 0.50 0.50 0.50 SnO₂ 0.23 0.23 0.23 0.23 0.23 0.23 0.23 0.47 0.00 CeO₂ 0.27 0.27 0.27 0.27 0.27 0.27 0.27 0.00 0.53 Fe₂O₃ 0.01 0.01 0.02 0.02 0.02 0.02 0.00 0.02 0.02

TABLE 3c Compositions of glasses prepared from crucible melts described in Example 3, expressed in mole percent. Composition (mol % ) 31 32 33 34 35 36 37 38 39 SiO₂ 65.89 65.89 65.89 65.89 65.89 65.89 65.89 65.89 65.89 Al₂O₃ (Alumina) 0 0 10.27 10.27 10.27 10.27 0 10.27 10.27 Al₂O₃ (Al(OH)₃) 10.27 10.27 0 0 0 0 0 0 0 Al₂O₃ (Nepheline) 0 0 0 0 0 0 10.27 0 0 B₂O₃ 0.63 0.63 0.63 0.63 0.63 0.63 0.63 0.63 0.63 Na₂O (Soda Ash) 13.91 13.91 11.91 11.91 12.91 9.91 11.91 11.91 11.91 Na₂O (NaNO₃) 0 0 2 2 1 4 2 2 2 K₂O 2.45 2.45 2.45 2.45 2.45 2.45 2.45 2.45 2.45 MgO 5.86 5.86 5.86 5.86 5.86 5.86 5.86 5.86 5.86 CaO 0.57 0.57 0.57 0.57 0.57 0.57 0.57 0.57 0.57 SnO₂ 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0.2 0 CeO₂ 0.10 0.10 0.10 0.10 0.10 0.10 0.10 0 0.2

TABLE 4a Compositions of batch materials, expressed in grams, for crucible melts described in Example 4. Batch Material 41 42 43 44 45 46 47 48 49 Sand 584.01 564.43 564.43 584.02 564.44 558.44 584.59 519.71 584.01 Alumina 13.55 13.59 13.58 13.54 13.58 13.44 13.67 13.71 13.55 Soda Ash 191.49 190.94 176.68 84.28 84.00 83.18 191.49 191.41 184.36 Sodium Nitrate 0.00 0.00 22.87 0.00 0.00 22.65 0.00 0.00 0.00 Magnesia 32.25 32.17 32.17 32.25 32.18 31.86 32.48 0 32.25 Limestone 104.02 103.88 103.91 104.28 104.14 102.96 0 104.25 104.03 Sodium hydroxide 0.00 0.00 0.00 81.25 81.04 80.21* 0.00 0.00 0.00 Lime hydrate 0.00 0.00 0.00 0.00 0.00 0.00 94.99 0.00 0.00 Talc 0.00 0.00 0.00 0.00 0.00 0.00 0.00 103.47 0.00 Tin (IV) Oxide 0.00 20.00 20.00 0.00 20.00 20.00 0.00 0.00 0.00 Sodium sulfate 0.00 0.00 0.00 0.00 0.00 0.00 0.00 0.00 9.53 *CaOH substituted for NaOH

TABLE 4b Compositions of glasses prepared from crucible melts described in Example 4, expressed in weight percent. Composition (wt %) 41 42 43 44 45 46 47 48 49 SiO₂ 72.94 72.75 72.75 72.94 72.75 72.00 72.94 72.86 72.46 Al₂O₃ 1.89 1.89 1.89 1.89 1.89 1.87 1.89 1.89 1.88 Na₂O 13.96 13.92 13.92 13.97 13.92 14.81 13.96 13.95 13.87 MgO 4.08 4.07 4.07 4.08 4.07 4.03 4.08 4.07 4.05 CaO 7.09 7.08 7.08 7.09 7.08 7.00 7.09 7.08 7.04 SnO₂ 0.00 0.25 0.25 0.00 0.25 0.25 0.00 0.00 0.00 SO₃ 0.00 0.00 0.00 0.00 0.00 0.00 0.00 0.00 0.67 Fe₂O₃ 0.04 0.04 0.04 0.04 0.04 0.04 0.05 0.15 0.04

TABLE 4c Compositions of glasses prepared from crucible melts described in Example 4, expressed in mole percent. Composition (mol %) 41 42 43 44 45 46 47 48 49 SiO₂ 72. 72. 72. 72. 72. 72. 72. 72. 72. Al₂O₃ 1.1 1.1 1.1 1.1 1.1 1.1 1.1 1.1 1.1 Na₂O (Soda Ash) 13.4 13.4 12.4 5.9 5.9 5.9 13.4 13.4 12.9 Na₂O (NaNO₃) 0 0 1 0 0 1 0 0 0 MgO 6 6 6 6 6 6 6 0 6 CaO 7.5 7.5 7.5 7.5 7.5 7.5 0 7.5 7.5 Na₂O 0 0 0 7.5 7.5 7.5 0 0 0 CaO 0 0 0 0 0 0 7.5 0 0 MgO 0 0 0 0 0 0 0 6 0 SnO₂ 0 0.1 0.1 0 0.1 0.1 0 0 0 Na₂O 0 0 0 0 0 0 0 0 .5

TABLE 5a Compositions of batch materials, expressed in grams, for crucible melts described in Example 5. Batch Material 51 52 53 54 55 56 57 58 59 Sand 555.02 555.04 555.06 553.96 553.92 552.82 550.55 623.69 623.73 Alumina 192.23 99.12 0 0 191.84 191.54 0 182.65 0 Alumina, hydrated 0 142.40 293.98 293.37 0 0 291.70 0 279.33 Magnesia 14.06 14.06 14.06 13.96 13.96 13.96 13.96 29.26 29.26 Limestone 59.39 59.39 59.39 59.39 59.39 59.21 59.02 79.24 79.24 Strontium carbonate 5.16 5.16 5.16 5.16 5.16 5.16 5.02 29.34 29.34 Barium carbonate 51.92 51.92 51.92 51.79 51.79 51.79 51.53 80.48 80.48 Lanthanum oxide 111.63 111.63 111.63 111.42 111.42 111.22 110.72 0 0 Yttrium oxide 29.40 29.40 29.40 29.30 29.30 29.30 29.20 0 0 Tin (IV) Oxide 2.01 2.01 2.01 3.91 3.91 5.92 1.91 2.21 2.21 Barium nitrate 34.32 34.32 34.32 34.15 34.15 34.15 33.97 38.61 38.61 Boric acid 0.00 0.00 0.00 0.00 0.00 0.00 0.00 22.70 22.70 Sodium hydroxide 9.81

TABLE 5b Compositions of glasses prepared from crucible melts described in Example 5, expressed in weight percent. Composition (wt %) 51 52 53 54 55 56 57 58 59 SiO₂ 54.74 54.74 54.74 54.65 54.64 54.52 54.31 61.45 61.45 Al₂O₃ 19.08 19.08 19.08 19.05 19.05 19.01 18.94 18.14 18.14 MgO 1.42 1.42 1.42 1.41 1.41 1.41 1.41 2.91 2.91 CaO 3.19 3.19 3.19 3.19 3.19 3.18 3.17 4.25 4.25 SrO 0.42 0.42 0.42 0.42 0.42 0.41 0.41 2.10 2.10 BaO 5.90 5.90 5.90 5.88 5.88 5.88 5.85 8.31 8.31 La₂O₃ 10.93 10.93 10.93 10.92 10.92 10.89 10.85 0.00 0.00 Y₂O₃ 2.90 2.90 2.90 2.89 2.89 2.89 2.88 0.00 0.00 SnO₂ 0.20 0.20 0.20 0.39 0.39 0.58 0.19 0.22 0.22 B₂O₃ 0.00 0.00 0.00 0.00 0.00 0.00 0.00 1.26 1.26 Na₂O 0.00 0.00 0.00 0.00 0.00 0.00 0.79 0.00 0.00 Fe₂O₃ 0.03 0.02 0.02 0.02 0.03 0.03 0.02 0.03 0.03 NO₂ 1.19 1.19 1.19 1.18 1.18 1.18 1.17 1.33 1.33 Cl— 0.01 0.01 0.01 0.01 0.01 0.01 0.01 0.00 0.00

TABLE 5c Compositions of glasses prepared from crucible melts described in Example 5, expressed in mole percent. Composition (mol %) 51 52 53 54 55 56 57 58 59 SiO₂ 70.86 70.86 70.86 70.86 70.86 70.86 70.86 70.6 70.6 Al₂O₃ 14.56 7.56 0 0 14.56 14.56 0 12.28 0 Al₂O₃ 0 7 14.56 14.56 0 0 14.56 0 12.28 MgO 2.74 2.74 2.74 2.74 2.74 2.74 2.74 4.99 4.99 CaO 4.43 4.43 4.43 4.43 4.43 4.43 4.43 5.23 5.23 SrO .31 .31 .31 .31 .31 .31 .31 1.40 1.40 BaO 1.99 1.99 1.99 1.99 1.99 1.99 1.99 2.74 2.74 La₂O₃ 2.61 2.61 2.61 2.61 2.61 2.61 2.61 0 0 Y₂O₃ 1.00 1.00 1.00 1.00 1.00 1.00 1.00 0 0 SnO₂ 0.10 0.10 0.10 0.2 0.2 0.3 0.10 0.10 0.10 BaO 1 1 1 1 1 1 1 1 1 B₂O₃ 0 0 0 0 0 0 0 1.25 1.25 Na₂O 0 0 0 0 0 0 1 0 0

TABLE 6a1 Compositions of batch materials, expressed in grams, for crucible melts described in Example 6. Batch Material 61 62 63 64 Sand 608.27 616.75 568.66 609.37 Alumina 84.32 72.69 81.04 173.87 Boric oxide 29.38 52.59 118.86 118.76 Soda Ash 199.39 176.49 98.95 82.7 Potassium carbonate 46.21 40.91 23.11 23.1 Lithium carbonate 10.49 21.23 52.2 51.95 Magnesia 29.26 22.14 −0.13 −0.14 Limestone 6.004 4.321 −0.48 −0.45 Tin (IV) oxide 0 0 46 0 Arsenic Pentoxide 0 0 0 6.986 Sodium nitrate 0 0 0 26.04 Alumina, hydrated 143.32 145 142.4 0

TABLE 6a2 Compositions of batch materials, expressed in grams, for crucible melts described in Example 6. Batch Material 66 67 Sand 350.12 350.11 Alumina 0 79.05 Alumina, hydrated 241.72 119.71 Boric acid 116.71 116.71 Soda ash 195.24 97.92 Sodium hydroxide 0 73.77 Potassium carbonate 57.69 57.69 Magnesia 15.07 15.07 Limestone 3.956 4.191 Tin (IV) oxide 230 230 Cerium (IV)oxide 26 26

TABLE 6b1 Compositions of glasses prepared from crucible melts of batch compositions listed in Table 6a1 and described in Example 6, expressed in weight percent. Composition (wt %) 61 62 63 64 SiO₂ 60.66 61.5 60.83 60.74 Al₂O₃ 17.89 16.84 17.49 17.46 B₂O₃ 2.9 5.19 11.73 11.72 Na₂O 11.69 10.35 5.82 5.81 K₂O 3.14 2.78 1.57 1.57 MgO 0.42 0.85 2.09 2.08 CaO 2.89 2.19 0 0 SnO₂ 0.39 0.29 0 0 As₂O₃ 0 0 0.46 0 SO₃ 0 0 0 0.6 Sb₂O₃ 0 0 0 0 Fe₂O₃ 0 0 0 0 H₂O 0.02 0.02 0.01 0.02 Cl— 0 0 0 0

TABLE 6b2 Compositions of glasses prepared from crucible melts of batch compositions listed in Table 6a2 and described in Example 6, expressed in weight percent. Composition (wt %) 65 66 SiO₂ 60.03 60.03 Al₂O₃ 15.77 15.77 B₂O₃ 6.58 6.58 Na₂O 11.45 11.45 K₂O 3.92 3.92 MgO 1.49 1.49 CaO 0.26 0.26 SnO₂ 0.23 0.23 CeO₂ 0.26 0.26 Fe₂O₃ 0.01 0.01 H₂O 0 0 Cl— 0 0

TABLE 6c1 Compositions of glasses prepared from crucible melts of batch compositions listed in Table 6a1 and described in Example 6, expressed in mole percent. Composition (mol %) 61 62 63 64 SiO₂ 66.04 66.21 66.7 66.7 Al₂O₃ 5.48 4.68 5.3 11.3 B₂O₃ 2.72 4.82 11.1 11.1 Na₂O 12.37 10.83 6.2 5.2 K₂O 2.18 1.91 1.1 1.1 Li₂O 0.92 1.84 4.6 4.6 MgO 4.69 3.52 0 0 SnO₂ 0 0 0.2 0 As₂O₃ 0 0 0 0.2 Na₂O 0 0 0 1 Al₂O₃ 6 6 6 0

TABLE 6c2 Compositions of glasses prepared from crucible melts of batch compositions listed in Table 6a2 and described in Example 6, expressed in mole percent. Composition (mol %) 65 66 SiO₂ 65.23 65.23 Al₂O₃ 0 5.1 Al₂O₃ 10.1 5 B₂O₃ 6.17 6.17 Na₂O 12.1 6.1 Na₂O 0 6 K₂O 2.72 2.72 MgO 2.41 2.41 CaO 0.3 0.3 SnO₂ 0.1 0.1 CeO₂ 0.1 0.1 

The invention claimed is:
 1. A method of making a silicate glass having a seed concentration of less than about 1 seed/cm³, wherein the method comprises: melting at a first temperature a glass batch comprising 60-70 mol % SiO₂; 6-14 mol % Al₂O₃; 0-3 mol % B₂O₃; 0-1 mol % Li₂O; 8-18 mol % Na₂O; 0-5 mol % K₂O; 0-2.5 mol % CaO; above 0 to 3 mol % ZrO₂; and a fining agent, wherein 12 mol %≤Li₂O +Na₂O+K₂O≤20 mol %, and wherein the glass batch comprises less than 50 ppm As₂O₃; and heating at a second temperature greater than the first temperature for a time sufficient to produce the silicate glass having a seed concentration of less than about 1 seed/cm³, wherein the fining agent is selected from the group consisting of SnO₂, CeO₂, and combinations thereof, and the fining agent comprises from 0-1 mol % SnO₂ and 0-1 mol % CeO₂ of the glass batch.
 2. The method of claim 1 wherein the first temperature is about 1425° C. to about 1550° C. and the second temperature is about 1525° C. to about 1675° C.
 3. The method of claim 1 wherein the difference between the second temperature and the first temperature is about 50° C. to about 250° C.
 4. The method of claim 3 wherein the difference between the second temperature and the first temperature is about 75° C. to about 100° C.
 5. The method of claim 1 wherein the glass batch comprises at least one inorganic compound that acts as of a source of H₂O at a temperature where a melt is formed.
 6. The method of claim 1 wherein the glass batch comprises an oxidizer fining agent.
 7. The method of claim 1 wherein the glass batch comprises fining agent selected from the group consisting of aluminum hydroxide, sodium hydroxide, or combinations thereof.
 8. The method of claim 1 further comprising ion exchanging the silicate glass to achieve a surface compressive stress of at least about 200 MPa and a surface compressive layer having a depth of at least about 30 μm.
 9. The method of claim 1 further comprising forming a glass sheet from the silicate glass via down-draw method.
 10. The method of claim 1, wherein the glass batch further comprises at least one clay or zeolite.
 11. The method of claim 1, wherein the glass batch further comprises aluminum silicate hydroxides, talc, montmorillonitesmectite, and combinations thereof.
 12. A method of making a silicate glass having a seed concentration of less than about 1 seed/cm³, wherein the method comprises: melting at a first temperature a glass batch comprising 60-70 mol % SiO₂; 0-3 mol % B₂O₃; 0-1 mol % Li₂O; 8-18 mol % Na₂O; 0-5 mol % K₂O; 0-2.5 mol % CaO; above 0 to 3% mol ZrO₂; and a fining agent, wherein 12 mol %<Li₂O+Na₂O+K₂O≤20 mol %, and wherein the glass batch is substantially free of As₂O₃; and heating at a second temperature greater than the first temperature for a time sufficient to produce the silicate glass having a seed concentration of less than about 1 seed/cm³, wherein the fining agent is selected from the group consisting of SnO₂, CeO₂, and combinations thereof, and the fining agent comprises 0-1 mol % SnO₂ and 0-1 mol % CeO₂ of the glass batch.
 13. The method of claim 12 wherein the first temperature is about 1425° C. to about 1550° C. and the second temperature is about 1525° C. to about 1675° C.
 14. The method of claim 12 wherein the difference between the second temperature and the first temperature is about 50° C. to about 250° C.
 15. The method of claim 14 wherein the difference between the second temperature and the first temperature is about 75° C. to about 100° C.
 16. The method of claim 12 wherein the glass batch comprises at least one inorganic compound that acts as of a source of H₂O at a temperature where a melt is formed.
 17. The method of claim 12 wherein the glass batch comprises an oxidizer fining agent.
 18. The method of claim 12 wherein the glass batch comprises fining agent selected from the group consisting of aluminum hydroxide, sodium hydroxide, or combinations thereof.
 19. The method of claim 12 further comprising ion exchanging the silicate glass to achieve a surface compressive stress of at least about 200 MPa and a surface compressive layer having a depth of at least about 30 μm.
 20. The method of claim 12 further comprising forming a glass sheet from the silicate glass via down-draw method.
 21. A method of making a silicate glass having a seed concentration of less than about 1 seed/cm³, wherein the method comprises: melting at a first temperature a glass batch comprising 60-70 mol % SiO₂; 6-14 mol % Al₂O₃; 0-15 mol % B₂O₃; 0-1 mol % Li₂O; 0-20 mol % Na₂O; 0-10 mol % K₂O; 0-10 mol % CaO; 0-5 mol % ZrO₂; wherein 12 mol %≤Li₂O+Na₂O+K₂O≤20 mol %, wherein the glass batch comprises less than 50 ppm As₂O₃, wherein the glass batch comprises a fining agent comprising a multivalent metal oxide, an oxidizer, and at least one inorganic compound that acts as of a source of water at a temperature where a melt is formed; and heating at a second temperature greater than the first temperature for a time sufficient to produce the silicate glass having a seed concentration of less than about 1 seed/cm³.
 22. The method of claim 21 wherein the first temperature is about 1425° C. to about 1550° C. and the second temperature is about 1525° C. to about 1675° C.
 23. The method of claim 21 wherein the difference between the second temperature and the first temperature is about 50° C. to about 250° C.
 24. The method of claim 23 wherein the difference between the second temperature and the first temperature is about 75° C. to about 100° C.
 25. The method of claim 21 wherein the glass batch comprises at least one inorganic compound that acts as of a source of H₂O at a temperature where a melt is formed.
 26. The method of claim 21 wherein the glass batch comprises an oxidizer fining agent.
 27. The method of claim 21 wherein the glass batch comprises fining agent selected from the group consisting of aluminum hydroxide, sodium hydroxide, or combinations thereof.
 28. The method of claim 21 further comprising ion exchanging the silicate glass to achieve a surface compressive stress of at least about 200 MPa and a surface compressive layer having a depth of at least about 30 μm.
 29. The method of claim 21 further comprising forming a glass sheet from the silicate glass via down-draw method.
 30. The method of claim 21 wherein the multivalent oxide fining agent is selected from the group consisting of SnO₂, CeO₂, and combinations thereof. 